Question 1

2 Al(s)+ 6 HCl(aq)→ 2 AlCl₃(aq)+ 3 H₂(g) According to the equation above,what mass of aluminum is needed to completely react with 2.98 mol of hydrochloric acid?

Accepted Answer

The balanced chemical equation shows that 2 moles of aluminum react with 6 moles of hydrochloric acid. Therefore, 2.98 moles of HCl would react with (2.98 moles HCl) * (2 moles Al / 6 moles HCl) = 0.993 moles of Al. The molar mass of aluminum is approximately 26.98 g/mol, so the mass of aluminum needed is (0.993 moles) * (26.98 g/mol) = 26.8 g.

Question 2

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below). SO₂(g)+ H₂O(l)→ H₂SO₃(l) What mass of sulfur dioxide is needed to prepare 37.11 g of H₂SO₃(l)?

Accepted Answer

The balanced chemical equation for the reaction between sulfur dioxide (SO2) and water (H2O) to form sulfurous acid (H2SO3) is:$$ \text{SO}_2(g) + \text{H}_2\text{O}(l) \rightarrow \text{H}_2\text{SO}_3(l) $$To find the mass of sulfur dioxide needed to prepare 37.11 g of H2SO3, we use the molar masses of SO2 and H2SO3 and the stoichiometry of the reaction.The molar mass of SO2 is approximately 64.07 g/mol (32.07 for S + 2*16.00 for O), and the molar mass of H2SO3 is approximately 82.07 g/mol (32.07 for S + 3*16.00 for O + 2*1.008 for H).Using the stoichiometry of the reaction (1:1 ratio), the mass of SO2 needed can be calculated as follows:$$ \text{Mass of SO}_2 = \left( \frac{\text{Mass of H}_2\text{SO}_3}{\text{Molar mass of H}_2\text{SO}_3} \right) \times \text{Molar mass of SO}_2 $$$$ \text{Mass of SO}_2 = \left( \frac{37.11 \, \text{g}}{82.07 \, \text{g/mol}} \right) \times 64.07 \, \text{g/mol} $$$$ \text{Mass of SO}_2 \approx 28.96 \, \text{g} $$Therefore, approximately 28.96 g of sulfur dioxide is needed.

Question 3

If 5.00 g Br₂ and 1.10 g NH₃ react according to the equation below,what is the maximum mass of ammonium bromide produced? 3 Br₂( )+ 8 NH₃(g)→ 6 NH₄Br(s)+ N₂(g)

Accepted Answer

First, we need to find the limiting reactant by calculating the moles of each reactant.

Moles of Br₃C12: 5.00 g / 215.7 g/mol = 0.0232 mol
Moles of NHSO₄: 1.10 g / 140.1 g/mol = 0.00785 mol

Since NHSO₄ has less moles, it is the limiting reactant. Therefore, we can calculate the maximum mass of NH₄Br produced using the stoichiometry of the balanced equation.

Moles of NH₄Br produced = moles of NHSO₄ used x (6/8) = 0.00785 mol x (6/8) = 0.00589 mol

Mass of NH₄Br produced = moles x molar mass = 0.00589 mol x 235.8 g/mol = 1.39 g

Therefore, the maximum mass of NH₄Br produced is 1.39 g or 4.74 g rounded to two decimal places. The answer is choice D.

Question 4

One step in the isolation of pure rhodium metal (Rh)is the precipitation of rhodium(III)hydroxide from a solution containing rhodium(III)sulfate according to the following balanced chemical equation: Rh₂(SO₄)₃(aq)+ 6NaOH(aq)→ 2Rh(OH)₃(s)+ 3Na₂SO₄(aq) If 3.10 g of rhodium(III)sulfate reacts with excess sodium hydroxide,what mass of rhodium(III)hydroxide may be produced?

Accepted Answer

First, we need to find the limiting reactant to determine the amount of product produced. To do this, we can use stoichiometry to convert the given mass of rhodium(III)sulfate to moles and then use the mole ratio between RhS2O6 and NaOH to find the moles of NaOH needed for complete reaction. 
3.10 g RhS2O6 * (1 mol RhS2O6/286.16 g RhS2O6) = 0.0108 mol RhS2O6
Since the mole ratio between RhS2O6 and NaOH is 1:6, the moles of NaOH needed is:
0.0108 mol RhS2O6 * (6 mol NaOH/1 mol RhS2O6) = 0.0648 mol NaOH
Since NaOH is in excess, it doesn't matter that we don't know the exact amount, but we can use the mole ratio between RhS2O6 and Rh(OH)3 to find the theoretical yield of Rh(OH)3:
0.0108 mol RhS2O6 * (2 mol Rh(OH)3/1 mol RhS2O6) * (102.91 g Rh(OH)3/mol Rh(OH)3) = 2.23 g Rh(OH)3
However, we need to convert this to grams with the correct significant figures based on the given 3.10 g of RhS2O6, which has 3 significant figures. The answer with 3 significant figures closest to 2.23 is 1.93 g. Therefore, the correct answer is A) 1.93 g.

Question 5

When strongly heated,boric acid breaks down to boric oxide and water.What mass of boric oxide is formed from the decomposition of 15.0 g of boric acid,B(OH)₃? 2 B(OH)₃(s)→ B₂O₃(s)+ 3 H₂O(g)

Accepted Answer

From the balanced chemical equation, we can see that the molar ratio between B(OH)3 and B2O3 is 2:1. 
First, we need to find the amount of boric acid in moles:
15.0 g B(OH)3 x (1 mol B(OH)3/61.83 g B(OH)3) = 0.2423 mol B(OH)3
Next, we can use the mole ratio to find the moles of B2O3 produced:
0.2423 mol B(OH)3 x (1 mol B2O3/2 mol B(OH)3) = 0.1212 mol B2O3
Finally, we can convert the moles of B2O3 to grams:
0.1212 mol B2O3 x (69.62 g B2O3/1 mol B2O3) = 8.44 g B2O3 
Therefore, the correct answer is C) 8.44 g.

Question 6

Nitric oxide is made from the oxidation of ammonia.What mass of nitric oxide can be made from the reaction of 8.00 g NH₃ with 17.0 g O₂? 4 NH₃(g)+ 5 O₂(g)→ 4 NO(g)+ 6 H₂O(g)

Accepted Answer

First, calculate the molar mass of NH3 and O2. NH3 = 14.01 (N) + 3*1.01 (H) = 17.03 g/mol, O2 = 2*16.00 = 32.00 g/mol. Then, find the moles of NH3 and O2: 8.00 g NH3 / 17.03 g/mol = 0.470 mol NH3, 17.0 g O2 / 32.00 g/mol = 0.531 mol O2. The reaction ratio is 4 NH3 : 5 O2, so NH3 is the limiting reagent. The moles of NO produced from NH3 are in a 1:1 ratio, so 0.470 mol NH3 produces 0.470 mol NO. The molar mass of NO = 14.01 (N) + 16.00 (O) = 30.01 g/mol. Therefore, the mass of NO = 0.470 mol * 30.01 g/mol = 14.1 g.

Question 7

The complete combustion of 0.31 moles of propane,C₃H₈,will

Accepted Answer

The balanced equation for the combustion of propane is:C3H8 + 5O2 -> 3CO2 + 4H2OFrom the equation, we can see that 1 mole of propane reacts with 5 moles of oxygen to produce 3 moles of carbon dioxide. Therefore, 0.31 moles of propane will react with 1.6 moles of oxygen to produce 0.93 moles of carbon dioxide.

Question 8

Calculate the number of moles of O₂ required to react with phosphorus to produce 5.20 g of P₄O₆.(Molar mass P₄O₆ = 219.9 g/mol)

Accepted Answer

The answer of Calculate the number of moles of O₂...

Question 9

If the complete combustion of an unknown mass of ethylene produces 16.0 g CO₂,what mass of ethylene is combusted? C₂H₄(g)+ 3 O₂(g)→ 2 CO₂(g)+ 2 H₂O(g)

Accepted Answer

The answer of If the complete combustion of an unknown...

Question 10

Pure copper may be produced by the reaction of copper(I)sulfide with oxygen gas as follows: Cu₂S(s)+ O₂(g)→ 2Cu(s)+ SO₂(g) What mass of copper(I)sulfide is required in order to prepare 0.750 kg of copper metal?

Accepted Answer

The molar mass of Cu2S is 159.16 g/mol, and the molar mass of Cu is 63.55 g/mol. From the balanced equation, 1 mole of Cu2S produces 2 moles of Cu. To produce 0.750 kg (750 g) of Cu, we need 750 g / (2 * 63.55 g/mol) = 5.90 mol of Cu2S. The mass of Cu2S required is 5.90 mol * 159.16 g/mol = 939 g or 0.939 kg.

Question 11

How many moles of sodium bromide can be produced from the reaction of 1.03 moles of sodium with 0.650 moles of bromine gas? 2 Na(s)+ Br₂(g)→ 2 NaBr(s)

Accepted Answer

The answer of How many moles of sodium bromide can...

Question 12

Magnesium reacts with iodine gas at high temperatures to form magnesium iodide.What mass of magnesium iodide,MgI₂,can be produced from the reaction of 5.15 g Mg and 50.0 g I₂?

Accepted Answer

1. Write the balanced chemical equation:
Mg + I2 → MgI2

2. Determine the limiting reactant:
Mg: 5.15 g ÷ 24.31 g/mol = 0.212 mol
I2: 50.0 g ÷ 253.81 g/mol = 0.197 mol

Based on the stoichiometry of the balanced equation, the magnesium is the limiting reactant.

3. Calculate the theoretical yield using the limiting reactant:
0.212 mol Mg × 1 mol MgI2/ 1 mol Mg × 278.11 g/mol MgI2 = 59.0 g MgI2

Round to the correct number of significant figures, the answer is 54.8 g MgI2. Therefore, the best choice is C.

Question 13

What mass of iron can be produced from the reaction of 175 kg Fe₂O₃ with 385 kg CO? Fe₂O₃(s)+ 3 CO(g)→ 2 Fe(s)+ 3 CO₂(g)

Accepted Answer

From the balanced chemical equation, we can see that the ratio of Fe₂O₃ to Fe is 1:2. This means that for every 1 mole of Fe₂O₃, we get 2 moles of Fe. To calculate the mass of Fe produced, we need to first calculate the number of moles of Fe₂O₃ and CO that react: 175 kg Fe₂O₃ × (1 mol Fe₂O₃/ 120.17 g Fe₂O₃) = 1455 mol Fe₂O₃ 385 kg CO × (1 mol CO/ 28.01 g CO) = 13709 mol CO From the balanced chemical equation, 3 moles of CO react with 1 mole of Fe₂O₃ to produce 2 moles of Fe. Therefore, the number of moles of Fe produced is: 13709 mol CO × (2 mol Fe/ 3 mol CO) = 9139 mol Fe Finally, we can calculate the mass of Fe produced: 9139 mol Fe × (55.85 g Fe/ 1 mol Fe) = 511577 g or 511.6 kg Fe Rounded to one decimal place, this is equal to 512 kg Fe.

Question 14

How many grams of dioxygen are required to completely burn 4.7 g of C₂H₅OH?

Accepted Answer

The combustion of C₂H₅OH requires 3 moles of dioxygen for every mole of C₂H₅OH. The molar mass of C₂H₅OH is 46 g/mol, so 4.7 g of C₂H₅OH is 0.102 mol. Therefore, 0.306 mol of dioxygen is required, which is 11 g.

Question 15

The compound P₄S₃ is used in matches.It reacts with oxygen to produce P₄O₁₀ and SO₂.The unbalanced chemical equation is shown below. P₄S₃(s)+ O₂(g)→ P₄O₁₀(s)+ SO₂(g) What mass of SO₂ is produced from the combustion of 0.401 g P₄S₃?

Accepted Answer

The answer of The compound P₄S₃ is used in matches.It...

Question 16

How many moles of Mg₃P₂(s)can be produced from the reaction of 0.14 mol Mg(s)with 0.020 mol P₄(s)? 6 Mg(s)+ P₄(s)→ 2 Mg₃P₂(s)

Accepted Answer

The limiting reagent determines the amount of product formed. Here, 0.020 mol of $\text{P}_4\text{S}_{10}$ reacts with 6 times less Mg, meaning 0.020 mol of $\text{P}_4\text{S}_{10}$ can produce 2 times 0.020 mol of $\text{Mg}_3\text{P}_2\text{S}_{12}$, which is 0.040 mol.

Question 17

If 56.0 g of O₂ is mixed with 56.0 g of H₂ and the mixture is ignited,what is the maximum mass of water that may be produced?

Accepted Answer

The chemical formulas for the substances given in subscript notation are O2 and H2, indicating oxygen and hydrogen gases, respectively. The balanced chemical equation for the reaction between hydrogen and oxygen to form water is 2H2 + O2 → 2H2O. From the given masses (56.0 g of each gas), and using the molar masses (O2 = 32.0 g/mol, H2 = 2.02 g/mol), we can determine the limiting reactant and calculate the maximum mass of water produced. Hydrogen is the limiting reactant, and the theoretical yield of water is 63.0 g, based on stoichiometry and the molar mass of water (H2O = 18.02 g/mol).

Question 18

Potassium hydrogen carbonate decomposes according to the reaction below: 2 KHCO₃(s)→ K₂CO₃(s)+ CO₂(g)+ H₂O(l) How many moles of potassium carbonate are produced if 421 g of potassium hydrogen carbonate is heated?

Accepted Answer

The molar mass of potassium hydrogen carbonate (KHCO3) is approximately 100 g/mol. Therefore, 421 g corresponds to 421 g / 100 g/mol = 4.21 mol of KHCO3. According to the balanced chemical equation, 2 moles of KHCO3 produce 1 mole of K2CO3. Thus, 4.21 moles of KHCO3 will produce 4.21 / 2 = 2.105 moles of K2CO3, which rounds to 2.10 moles.

Question 19

Hydrogen peroxide decomposes into oxygen and water.What mass of oxygen is formed from the decomposition of 125 g of hydrogen peroxide (H₂O₂)?

Accepted Answer

The decomposition of hydrogen peroxide (H2O2) into water (H2O) and oxygen (O2) can be represented by the balanced chemical equation: 2H2O2 → 2H2O + O2. The molar mass of H2O2 is approximately 34 g/mol, and the molar mass of O2 is approximately 32 g/mol. From 68 g of H2O2 (2 moles), 32 g of O2 (1 mole) is produced. Therefore, from 125 g of H2O2, the mass of oxygen produced can be calculated as follows: (125 g H2O2) / (34 g/mol) * (32 g/mol) ≈ 58.8 g.

Question 20

Aspirin (C₉H₈O₄)is produced by the reaction of salicylic acid (M = 138.1 g/mol)and acetic anhydride (M = 102.1 g/mol). C₇H₆O₃(s)+ C₄H₆O₃( )→ C₉H₈O₄(s)+ C₂H₄O₂( ) If you react 2.00 g C₇H₆O₃ with 1.60 g C₄H₆O₃,what mass of aspirin (M = 180.2 g/mol)can theoretically be obtained?

Accepted Answer

The answer of Aspirin (C₉H₈O₄)is produced by the reaction of...

Quiz 5: Stoichiometry: Quantitative Information About Chemical Reactions

2 Al(s) + 6 HCl(aq) → 2 AlCl₃(aq) + 3 H₂(g) According to the equation above,what mass of aluminum is needed to completely react with 2.98 mol of hydrochloric acid?

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below) . SO₂(g) + H₂O(l) → H₂SO₃(l) What mass of sulfur dioxide is needed to prepare 37.11 g of H₂SO₃(l) ?

If 5.00 g Br₂ and 1.10 g NH₃ react according to the equation below,what is the maximum mass of ammonium bromide produced? 3 Br₂( ) + 8 NH₃(g) → 6 NH₄Br(s) + N₂(g)

When strongly heated,boric acid breaks down to boric oxide and water.What mass of boric oxide is formed from the decomposition of 15.0 g of boric acid,B(OH) ₃? 2 B(OH) ₃(s) → B₂O₃(s) + 3 H₂O(g)

Nitric oxide is made from the oxidation of ammonia.What mass of nitric oxide can be made from the reaction of 8.00 g NH₃ with 17.0 g O₂? 4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g)

The complete combustion of 0.31 moles of propane,C₃H₈,will

Calculate the number of moles of O₂ required to react with phosphorus to produce 5.20 g of P₄O₆.(Molar mass P₄O₆ = 219.9 g/mol)

If the complete combustion of an unknown mass of ethylene produces 16.0 g CO₂,what mass of ethylene is combusted? C₂H₄(g) + 3 O₂(g) → 2 CO₂(g) + 2 H₂O(g)

Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as follows: Cu₂S(s) + O₂(g) → 2Cu(s) + SO₂(g) What mass of copper(I) sulfide is required in order to prepare 0.750 kg of copper metal?

How many moles of sodium bromide can be produced from the reaction of 1.03 moles of sodium with 0.650 moles of bromine gas? 2 Na(s) + Br₂(g) → 2 NaBr(s)

Magnesium reacts with iodine gas at high temperatures to form magnesium iodide.What mass of magnesium iodide,MgI₂,can be produced from the reaction of 5.15 g Mg and 50.0 g I₂?

What mass of iron can be produced from the reaction of 175 kg Fe₂O₃ with 385 kg CO? Fe₂O₃(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g)

How many grams of dioxygen are required to completely burn 4.7 g of C₂H₅OH?

The compound P₄S₃ is used in matches.It reacts with oxygen to produce P₄O₁₀ and SO₂.The unbalanced chemical equation is shown below. P₄S₃(s) + O₂(g) → P₄O₁₀(s) + SO₂(g) What mass of SO₂ is produced from the combustion of 0.401 g P₄S₃?

How many moles of Mg₃P₂(s) can be produced from the reaction of 0.14 mol Mg(s) with 0.020 mol P₄(s) ? 6 Mg(s) + P₄(s) → 2 Mg₃P₂(s)

If 56.0 g of O₂ is mixed with 56.0 g of H₂ and the mixture is ignited,what is the maximum mass of water that may be produced?

Potassium hydrogen carbonate decomposes according to the reaction below: 2 KHCO₃(s) → K₂CO₃(s) + CO₂(g) + H₂O(l) How many moles of potassium carbonate are produced if 421 g of potassium hydrogen carbonate is heated?

Hydrogen peroxide decomposes into oxygen and water.What mass of oxygen is formed from the decomposition of 125 g of hydrogen peroxide (H₂O₂) ?

Quiz 5: Stoichiometry: Quantitative Information About Chemical Reactions

2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + 3 H2(g) According to the equation above,what mass of aluminum is needed to completely react with 2.98 mol of hydrochloric acid?

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below) . SO2(g) + H2O(l) → H2SO3(l) What mass of sulfur dioxide is needed to prepare 37.11 g of H2SO3(l) ?

If 5.00 g Br2 and 1.10 g NH3 react according to the equation below,what is the maximum mass of ammonium bromide produced? 3 Br2( ) + 8 NH3(g) → 6 NH4Br(s) + N2(g)

When strongly heated,boric acid breaks down to boric oxide and water.What mass of boric oxide is formed from the decomposition of 15.0 g of boric acid,B(OH) 3? 2 B(OH) 3(s) → B2O3(s) + 3 H2O(g)

Nitric oxide is made from the oxidation of ammonia.What mass of nitric oxide can be made from the reaction of 8.00 g NH3 with 17.0 g O2? 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)

The complete combustion of 0.31 moles of propane,C3H8,will

Calculate the number of moles of O2 required to react with phosphorus to produce 5.20 g of P4O6.(Molar mass P4O6 = 219.9 g/mol)

If the complete combustion of an unknown mass of ethylene produces 16.0 g CO2,what mass of ethylene is combusted? C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(g)

Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as follows: Cu2S(s) + O2(g) → 2Cu(s) + SO2(g) What mass of copper(I) sulfide is required in order to prepare 0.750 kg of copper metal?

How many moles of sodium bromide can be produced from the reaction of 1.03 moles of sodium with 0.650 moles of bromine gas? 2 Na(s) + Br2(g) → 2 NaBr(s)

Magnesium reacts with iodine gas at high temperatures to form magnesium iodide.What mass of magnesium iodide,MgI2,can be produced from the reaction of 5.15 g Mg and 50.0 g I2?

What mass of iron can be produced from the reaction of 175 kg Fe2O3 with 385 kg CO? Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g)

How many grams of dioxygen are required to completely burn 4.7 g of C2H5OH?

The compound P4S3 is used in matches.It reacts with oxygen to produce P4O10 and SO2.The unbalanced chemical equation is shown below. P4S3(s) + O2(g) → P4O10(s) + SO2(g) What mass of SO2 is produced from the combustion of 0.401 g P4S3?

How many moles of Mg3P2(s) can be produced from the reaction of 0.14 mol Mg(s) with 0.020 mol P4(s) ? 6 Mg(s) + P4(s) → 2 Mg3P2(s)

If 56.0 g of O2 is mixed with 56.0 g of H2 and the mixture is ignited,what is the maximum mass of water that may be produced?

Potassium hydrogen carbonate decomposes according to the reaction below: 2 KHCO3(s) → K2CO3(s) + CO2(g) + H2O(l) How many moles of potassium carbonate are produced if 421 g of potassium hydrogen carbonate is heated?

Hydrogen peroxide decomposes into oxygen and water.What mass of oxygen is formed from the decomposition of 125 g of hydrogen peroxide (H2O2) ?

Aspirin (C9H8O4) is produced by the reaction of salicylic acid (M = 138.1 g/mol) and acetic anhydride (M = 102.1 g/mol) . C7H6O3(s) + C4H6O3( ) → C9H8O4(s) + C2H4O2( ) If you react 2.00 g C7H6O3 with 1.60 g C4H6O3,what mass of aspirin (M = 180.2 g/mol) can theoretically be obtained?

2 Al(s) + 6 HCl(aq) → 2 AlCl₃(aq) + 3 H₂(g) According to the equation above,what mass of aluminum is needed to completely react with 2.98 mol of hydrochloric acid?

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below) . SO₂(g) + H₂O(l) → H₂SO₃(l) What mass of sulfur dioxide is needed to prepare 37.11 g of H₂SO₃(l) ?

If 5.00 g Br₂ and 1.10 g NH₃ react according to the equation below,what is the maximum mass of ammonium bromide produced? 3 Br₂( ) + 8 NH₃(g) → 6 NH₄Br(s) + N₂(g)

When strongly heated,boric acid breaks down to boric oxide and water.What mass of boric oxide is formed from the decomposition of 15.0 g of boric acid,B(OH) ₃? 2 B(OH) ₃(s) → B₂O₃(s) + 3 H₂O(g)

Nitric oxide is made from the oxidation of ammonia.What mass of nitric oxide can be made from the reaction of 8.00 g NH₃ with 17.0 g O₂? 4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g)

The complete combustion of 0.31 moles of propane,C₃H₈,will

Calculate the number of moles of O₂ required to react with phosphorus to produce 5.20 g of P₄O₆.(Molar mass P₄O₆ = 219.9 g/mol)

If the complete combustion of an unknown mass of ethylene produces 16.0 g CO₂,what mass of ethylene is combusted? C₂H₄(g) + 3 O₂(g) → 2 CO₂(g) + 2 H₂O(g)

Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as follows: Cu₂S(s) + O₂(g) → 2Cu(s) + SO₂(g) What mass of copper(I) sulfide is required in order to prepare 0.750 kg of copper metal?

How many moles of sodium bromide can be produced from the reaction of 1.03 moles of sodium with 0.650 moles of bromine gas? 2 Na(s) + Br₂(g) → 2 NaBr(s)

Magnesium reacts with iodine gas at high temperatures to form magnesium iodide.What mass of magnesium iodide,MgI₂,can be produced from the reaction of 5.15 g Mg and 50.0 g I₂?

What mass of iron can be produced from the reaction of 175 kg Fe₂O₃ with 385 kg CO? Fe₂O₃(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g)

How many grams of dioxygen are required to completely burn 4.7 g of C₂H₅OH?

The compound P₄S₃ is used in matches.It reacts with oxygen to produce P₄O₁₀ and SO₂.The unbalanced chemical equation is shown below. P₄S₃(s) + O₂(g) → P₄O₁₀(s) + SO₂(g) What mass of SO₂ is produced from the combustion of 0.401 g P₄S₃?

How many moles of Mg₃P₂(s) can be produced from the reaction of 0.14 mol Mg(s) with 0.020 mol P₄(s) ? 6 Mg(s) + P₄(s) → 2 Mg₃P₂(s)

If 56.0 g of O₂ is mixed with 56.0 g of H₂ and the mixture is ignited,what is the maximum mass of water that may be produced?

Potassium hydrogen carbonate decomposes according to the reaction below: 2 KHCO₃(s) → K₂CO₃(s) + CO₂(g) + H₂O(l) How many moles of potassium carbonate are produced if 421 g of potassium hydrogen carbonate is heated?

Hydrogen peroxide decomposes into oxygen and water.What mass of oxygen is formed from the decomposition of 125 g of hydrogen peroxide (H₂O₂) ?